Hydrogen peroxide (H2O2, 34 g/mol) decomposes into water vapor and oxygen gas. How many liters of water vapor are produced from the decomposition of 17.0 g of H2O2 at STP?

The volume of water vapor produced at STP is 11.60 L.

Explanation:

The decomposition reaction of H₂O₂ is:

2H₂O₂ → O₂ + 2H₂O     (1)

We have:

m(H₂O₂): mass = 17.0 g

M(H₂O₂): molar mass = 34 g/mol    

To find the volume of water vapor produced we need to find first the number of moles of H₂O₂ and H₂O:

From the reaction (1) we have that 2 moles of H₂O₂ produce 2 moles of H₂O, so the number of moles of H₂O is:

Now, we can find the volume of water vapor produced at STP, using Ideal gas law:

Therefore, the volume of water vapor produced at STP is 11.60 L.

I hope it helps you!

i'm assuming that it's c.) red bank..

answer: semi-infinite solid initially at a uniform temperature of 400 ◦c is cooled at its surface by convection. the cooling fluid at a constant temperature of 200 ◦c has a convective coefficient (ha) of 250 w/m2.k. the physical properties of the solid: k = 20 w/m.k and α = 4 * 10-5  m2/s. using δx = 0.04 m and δt = 10 s. write the finite difference equations describing the transient heat transfer of the first five δx and the temperature profile after 30 s.